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Determine the types/s of intermolecular for systems. 1. K'and H20 2. C6H14 3. C6H14 and H20 4. CH3 CH2OH 5. H2S and HBr

Determine the types/s of intermolecular for systems. 1. K'and H20 2. C6H14 3. C6H14 and H20 4. CH3 CH2OH 5. H2S and HBr

World of Chemistry, 3rd edition
World of Chemistry, 3rd edition
3rd Edition
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Chapter14: Liquids And Solids
Section: Chapter Questions
Problem 3A
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Determine the types/s of intermolecular forces that exist in each of the following systems. 1. K'and H20 6. Hzand Br2 2. C6H14 7. SO2 3. C6H14 and H20 8. NazSO4 and H20 4. CH3 CH2OH 9. CH3COOH and H20 5. H2S and HBr 10. Cl and C6H14
Transcribed Image Text:Determine the types/s of intermolecular forces that exist in each of the following systems. 1. K'and H20 6. Hzand Br2 2. C6H14 7. SO2 3. C6H14 and H20 8. NazSO4 and H20 4. CH3 CH2OH 9. CH3COOH and H20 5. H2S and HBr 10. Cl and C6H14
ABSTRACTION (DISCUSSION PROPER) Intermolecular Forces of Attraction The attractive forces between nelghboring particles (Including molecules, atoms and lonsi are called intermolecular forces, Intermolecular forces can be Van der Waals forces, interactions between neutral molecules, namely dipole-dipole interaction. Dipole-induced dipole, and dispersion forces. It can also be jon-dipole, ion-induced dipole, and hydrogen bonding. 1. Dipole-dipole Interaction mis type of attraction exists between two polar molecules. As discussed in chemical bonding, polar molecules are formed when electrons are shared unequally, resulting in one atom being partially negative (-) and other being partially positive (+). Electronegativity property of an element determines to which atom shared electrons are closer. Examples: H20 ( H is partially + and O is partially -) CH3OH (C and H are partially + and O is partially -) 2. Dipole-induced Dipole Interaction For polar and nonpolar molecules, an interaction called dipole-induced dipole exists. In the presence of a polar molecule, a nonpolar molecule is forced to become a dipole. The polar molecule in a nearby nonpolar molecule causes the electrons of the latter to be distributed on one side allowing the other side to or positive (or to be distorted an induced dipole). Examples: H20 and Xe 3. Dispersion Forces Dispersion forces, also known as London Forces, exist in both polar and nonpolar molecules or in molecular compounds formed via equal sharing of electron (i.e. H2, F2, Cl2, Br2, O2, N2, CHA, CCI4). These forces arise temporarily when the electrons move in a direction away from the nucleus, resulting in an induced dipole within molecule. The creation o induced dipole allows attraction between two molecules. 4. lon-dipole Attraction The lon-dipole attraction exists between an ion and polar molecule. However, the strength of the interaction depends on the charge and size of the ion, the magnitude of the dipole moment, and the size of the molecule. Polar molecules can dissolve ionic compounds such as NaCl as a result of ion-dipole interaction. Examples: NaCl 5. lon-Induced Dipole Interaction The formation of induced dipole can also be caused by an approach of ions in the nonpolar molecule. This attractive between ion and the induced dipole (nonpolar) is called ion-induced dipole. Examples: Na and H20 6. Hydrogen Bonding Hydrogen bonding is a special type of dipole-dipole interaction. It exists in polar molecules that contain an H atom covalently bonded to highly electronegative atoms such as F, O and N. Being attached to N, O, and F hydrogen becomes positive because of the pull of the adjacent atom for the shared electrons.
Transcribed Image Text:ABSTRACTION (DISCUSSION PROPER) Intermolecular Forces of Attraction The attractive forces between nelghboring particles (Including molecules, atoms and lonsi are called intermolecular forces, Intermolecular forces can be Van der Waals forces, interactions between neutral molecules, namely dipole-dipole interaction. Dipole-induced dipole, and dispersion forces. It can also be jon-dipole, ion-induced dipole, and hydrogen bonding. 1. Dipole-dipole Interaction mis type of attraction exists between two polar molecules. As discussed in chemical bonding, polar molecules are formed when electrons are shared unequally, resulting in one atom being partially negative (-) and other being partially positive (+). Electronegativity property of an element determines to which atom shared electrons are closer. Examples: H20 ( H is partially + and O is partially -) CH3OH (C and H are partially + and O is partially -) 2. Dipole-induced Dipole Interaction For polar and nonpolar molecules, an interaction called dipole-induced dipole exists. In the presence of a polar molecule, a nonpolar molecule is forced to become a dipole. The polar molecule in a nearby nonpolar molecule causes the electrons of the latter to be distributed on one side allowing the other side to or positive (or to be distorted an induced dipole). Examples: H20 and Xe 3. Dispersion Forces Dispersion forces, also known as London Forces, exist in both polar and nonpolar molecules or in molecular compounds formed via equal sharing of electron (i.e. H2, F2, Cl2, Br2, O2, N2, CHA, CCI4). These forces arise temporarily when the electrons move in a direction away from the nucleus, resulting in an induced dipole within molecule. The creation o induced dipole allows attraction between two molecules. 4. lon-dipole Attraction The lon-dipole attraction exists between an ion and polar molecule. However, the strength of the interaction depends on the charge and size of the ion, the magnitude of the dipole moment, and the size of the molecule. Polar molecules can dissolve ionic compounds such as NaCl as a result of ion-dipole interaction. Examples: NaCl 5. lon-Induced Dipole Interaction The formation of induced dipole can also be caused by an approach of ions in the nonpolar molecule. This attractive between ion and the induced dipole (nonpolar) is called ion-induced dipole. Examples: Na and H20 6. Hydrogen Bonding Hydrogen bonding is a special type of dipole-dipole interaction. It exists in polar molecules that contain an H atom covalently bonded to highly electronegative atoms such as F, O and N. Being attached to N, O, and F hydrogen becomes positive because of the pull of the adjacent atom for the shared electrons.
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